Calculate the emf of the following cell at 25°C . [Fe | Fe^2+ (0.001M)|| H+ (0.01M) | H_2(g) (1bar) |Pt(s)]. E°(Fe2+/Fe= -0.44V), E°(H+/H=0.00V).
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For the given cell representation, the cell reaction will be
Fe(s)+2H+(aq)→Fe2+(aq)+H2(g)
The standard emf of the cell will be
Ecell∘=EH−+/H2∘−EFe2+/Fe∘
Ecell∘=0−(−0.44)=0.4
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